What volume of air containing 21% of oxygen (by volume) is required to completely burn 10g of sulphur which has a purity level of 98%.
3 answers
The volume of air required to completely burn 10g of sulphur with a purity level of 98% is approximately 5.2L. This is calculated by multiplying the mass of sulphur (10g) by the molar mass of sulphur (32.06 g/mol) to get the moles of sulphur (0.312 mol). Then, multiply the moles of sulphur by the molar volume of oxygen (22.4 L/mol) to get the volume of oxygen required (7.0 L). Finally, multiply the volume of oxygen required by the percentage of oxygen in the air (21%) to get the total volume of air required (5.2 L).
lots of words, but basically devoid of content
oobleck is right on. I think the questions (most of them anyway) are made up too.
3 answers